What is the term for the lowest energy state of an atom?

The term for the lowest energy state of an atom is known as the ground state. In this state, the electrons occupy the lowest available energy levels, which corresponds to the most stable configuration for the atom.

When an atom is in its ground state, it has the minimum amount of energy required to keep the electrons in their respective orbits around the nucleus. This state is fundamental because any addition of energy to the atom can promote one or more of its electrons to higher energy levels, resulting in an excited state.

The concept of an excited state refers specifically to these higher energy configurations, where electrons are elevated to energy levels above their ground state positions.

The ionized state describes an atom that has lost one or more of its electrons, which also indicates it is no longer in its ground state. In contrast, a stable state may imply that the atom has reached a configuration that does not change over time but does not specifically denote the lowest energy condition.

Thus, understanding that the ground state represents the baseline energy configuration is essential in the study of atomic structure and behavior.